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The p-Block Elements

Short Answer Type

591. Knowing the electron gain enthalpy values for O

\to

O^– and O

\to

O²^–as -141 and 702 kJ mol^–1 respectively, how can you account for the formation of a large number of oxides having O^2-species and not O^–?

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Long Answer Type

592. Using VSEPR theory, predict the structures of SO₃,²^– IF₇^–, XeF₂, ClO₄^–, ICl₄^– and IBr₂^–.

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Short Answer Type

593.
Assign a reason for each of the following statement:
Ammonia is a stronger base than phosphine.

This is because of the electronegitivity and size difference in the elements N and P. N has a higher electronegitivity and pulls the electrons in the N-H bonds toward itself, creating a more polar bond than the P-H bond. N is smaller than P thus it is a better lewis base, being able to form more stable sigma bonds. Both of these things cause NH₃is more basic than PH₃

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Long Answer Type

594. Draw the structures of the following molecules (i) SF₄, (ii) XeF₄.

264 Views

One Word Answers

595. Answer the following:
Of Bi(V) and Sb(V) which may be a stronger oxidising agent and why?

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Short Answer Type

596. Assign a reason for the following statement?
Phosphorus shows marked tendency for catenation but nitrogen shows little tendency for catenation.

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597. Assign a reason for the following statement?
The electron gain enthalpy with negative sign for oxygen (–141'k] mol–¹) is less that for sulphur (–200 kj mol^{– 1}).

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